Chapter 3, Problem 3.32E

Interpretation Introduction

Interpretation:

The abbreviated electronic configuration for all elements in which the noble gas symbol $\left[\text{Ne}\right]$ used are to be stated.

Concept introduction:

The elements in a modern periodic table are arranged in an increasing order of their atomic number. In the modern periodic table, the horizontal rows are known as periods, whereas vertical columns are known as groups. There are $7$ periods and $18$ groups in a modern periodic table.

Answer to Problem 3.32E

The abbreviated electronic configuration for all elements in which the noble gas symbol $\left[\text{Ne}\right]$ used are,

$\begin{array}{rllll}\text{Na}\left(11\right)& =& \left[\text{Ne}\right]3s^1\text{Mg}\left(12\right)& =& \left[\text{Ne}\right]3s^2\\ \text{Al}\left(13\right)& =& \left[\text{Ne}\right]3s^{2}3p^1\text{Si}\left(14\right)& =& \left[\text{Ne}\right]3s^{2}3p^2\\ \text{P}\left(15\right)& =& \left[\text{Ne}\right]3s^{2}3p^3\text{S}\left(16\right)& =& \left[\text{Ne}\right]3s^{2}3p^4\\ \text{Cl}\left(17\right)& =& \left[\text{Ne}\right]3s^{2}3p^5\text{Ar}\left(18\right)& =& \left[\text{Ne}\right]3s^{2}3p^6\end{array}$

Explanation of Solution

Neon is a noble gas and has $10$ electrons. The electronic configuration of neon is $1s^{2}2s^{2}2p^6$. After neon, argon is the next noble gas. The elements including argon after neon have $\left[\text{Ne}\right]$ in their abbreviated electronic configuration. Argon has $18$ electrons. Therefore, the elements that have number of electrons between $10$ to less than or equal to $18$ have $\left[\text{Ne}\right]$ in their abbreviated electronic configuration. Thus, there are $\text{8}$ elements that have $\left[\text{Ne}\right]$ in their abbreviated electronic configurations. The abbreviated electronic configuration for $\text{8}$ elements in which the noble gas symbol $\left[\text{Ne}\right]$ used is as follows:

$\begin{array}{rllll}\text{Na}\left(11\right)& =& \left[\text{Ne}\right]3s^1\text{Mg}\left(12\right)& =& \left[\text{Ne}\right]3s^2\\ \text{Al}\left(13\right)& =& \left[\text{Ne}\right]3s^{2}3p^1\text{Si}\left(14\right)& =& \left[\text{Ne}\right]3s^{2}3p^2\\ \text{P}\left(15\right)& =& \left[\text{Ne}\right]3s^{2}3p^3\text{S}\left(16\right)& =& \left[\text{Ne}\right]3s^{2}3p^4\\ \text{Cl}\left(17\right)& =& \left[\text{Ne}\right]3s^{2}3p^5\text{Ar}\left(18\right)& =& \left[\text{Ne}\right]3s^{2}3p^6\end{array}$

Conclusion

The abbreviated electronic configuration for all elements in which the noble gas symbol $\left[\text{Ne}\right]$ used are,

$\begin{array}{rllll}\text{Na}\left(11\right)& =& \left[\text{Ne}\right]3s^1\text{Mg}\left(12\right)& =& \left[\text{Ne}\right]3s^2\\ \text{Al}\left(13\right)& =& \left[\text{Ne}\right]3s^{2}3p^1\text{Si}\left(14\right)& =& \left[\text{Ne}\right]3s^{2}3p^2\\ \text{P}\left(15\right)& =& \left[\text{Ne}\right]3s^{2}3p^3\text{S}\left(16\right)& =& \left[\text{Ne}\right]3s^{2}3p^4\\ \text{Cl}\left(17\right)& =& \left[\text{Ne}\right]3s^{2}3p^5\text{Ar}\left(18\right)& =& \left[\text{Ne}\right]3s^{2}3p^6\end{array}$